The dependence of the equilibrium constant on temperature is given by the integrated Van't Hoff equa — Chemical Equilibrium Chemistry Question
Question
The dependence of the equilibrium constant $K$ on temperature $T$ is given by the integrated Van't Hoff equation: $\log_{10}\left(\frac{K_2}{K_1}\right) = \frac{\Delta H^\circ}{2.303R} \left[\frac{T_2 - T_1}{T_1 T_2}\right]$. Which of the following deductions are correct assuming $T_2 > T_1$?
Answer: A,B,C
💡 Solution & Explanation
If $T_2 > T_1$, the term $(T_2-T_1)/(T_1 T_2)$ is positive. For an endothermic reaction ($\Delta H^\circ > 0$), the right side is positive, making $\log(K_2/K_1) > 0$ and $K_2 > K_1$. For an exothermic reaction ($\Delta H^\circ < 0$), it is negative, so $K_2 < K_1$. If $\Delta H^\circ = 0$, $K_2 = K_1$. Option D is false because the slope is $-\Delta H^\circ / (2.303 R)$ due to the base-10 logarithm.
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